Net Ionic Equations and Solubility

This video tutorial explains how to write a balanced net ionic equation for the reaction between copper(II) chloride and sodium carbonate. It covers balancing the molecular equation, determining the solubility and states of substances, forming the complete ionic equation, and identifying spectator ions to derive the net ionic equation. The tutorial emphasizes the importance of charge conservation and atom balance in chemical equations.

What is the first step in writing a net ionic equation?

• Identify spectator ions

• Split compounds into ions

• Balance the molecular equation

• Determine the solubility of compounds

Why is it important to know the solubility rules when writing net ionic equations?

• To balance the equation

• To determine which compounds form precipitates

• To find the charge of ions

• To identify spectator ions

Which of the following compounds is generally insoluble?

• Sodium chloride

• Copper(II) carbonate

• Ammonium carbonate

• Potassium carbonate

What is the charge of the carbonate ion?

• 1-

• 2+

• 2-

• 1+

In the complete ionic equation, which ions are not split apart?

• Gaseous compounds

• Spectator ions

• Solid precipitates

• Aqueous ions

What are spectator ions?

• Ions that participate in the reaction

• Ions that are not present in the products

• Ions that do not change during the reaction

• Ions that form a precipitate

Which ions are considered spectator ions in the reaction between copper(II) chloride and sodium carbonate?

• Copper ions

• Carbonate ions

• Chloride ions

• Sodium ions

What is the net charge of the balanced net ionic equation?

• 1+

• 2+

• 0

• 2-

Why is it important to ensure that the charges are balanced in a net ionic equation?

• To determine solubility

• To ensure the equation is correct

• To identify spectator ions

• To find the molecular formula

What is the final step in writing a net ionic equation?

• Balancing the molecular equation

• Identifying spectator ions

• Ensuring charge and atom balance

• Determining solubility